- 220.127.116.11: Why is the formula shown for nitromethane incorrect?
- 18.104.22.168: The following inorganic species will be encountered in this text. C...
- 22.214.171.124: Calculate the formal charge on each nitrogen in the following Lewis...
Solutions for Chapter 1.6: Formal Charge
Full solutions for Organic Chemistry, | 9th Edition
A carbon atom adjacent to a carbonyl group
The SI unit of radioactivity. It corresponds to one nuclear disintegration per second. (Section 21.4)
boiling-point elevation (DTb).
The boiling point of the solution (Tb) minus the boiling point of the pure solvent (T° b). (12.6)
The enthalpy change required to break a bond in a mole of gaseous molecules. (9.10)
The ability of the atoms of an element to form bonds with one another. (22.3)
A tetrahedral atom, most commonly carbon, that is bonded to four different groups; also called a chirality center
A compound containing a cyano group and a hydroxyl group connected to the same carbon atom.
Dalton’s law of partial pressures
A law stating that the total pressure of a mixture of gases is the sum of the pressures that each gas would exert if it were present alone. (Section 10.6)
A compound containing two carbon-carbon p bonds.
A chemical formula that shows the kinds of atoms and their relative numbers in a substance in the smallest possible whole-number ratios. (Section 2.6)
A crystal lattice in which the lattice points are located at the faces and corners of each unit cell. (Section 12.2)
Le Châtelier’s principle
A principle stating that when we disturb a system at chemical equilibrium, the relative concentrations of reactants and
A compound thatrotates plane-polarized light in a counterclockwisedirection (-).
An equation that relates the cell emf, E, to the standard emf, E°, and the reaction quotient, Q: E = E° - 1RT>nF2 ln Q. (Section 20.6)
The name given to O3, an allotrope of oxygen. (Section 7.8)
In mass spectrometry,the ion that is generated when the compound is ionized.
The negative log in base 10 of the aquated hydrogen ion concentration: pH = -log3H+4. (Section 16.4)
Separation of a racemic mixture into its enantiomers; in mass spectrometry, a measure of how well a mass spectrometer separates ions of different mass.
A geometry adopted by an atom with a steric number of 3. All three groups lie in one plane and are separated by 120°.
A rule stating that the major product of a b-elimination reaction is the most stable alkene; that is, it is the alkene with the greatest number of substituents on the carboncarbon double bond